Self assembled multi-layer nanocomposite of graphene and metal oxide materials

ABSTRACT

Nanocomposite materials having at least two layers, each layer consisting of one metal oxide bonded to at least one graphene layer were developed. The nanocomposite materials will typically have many alternating layers of metal oxides and graphene layers, bonded in a sandwich type construction and will be incorporated into an electrochemical or energy storage device.

The invention was made with Government support under Contract DE-AC0676RLO 1830, awarded by the U.S. Department of Energy. The Government has certain rights in the invention.

TECHNICAL FIELD

This invention relates to nanocomposite materials of graphene bonded to metal oxides, devices using such materials, methods for forming nanocomposite materials of graphene bonded to metal oxides, and devices using those materials. More specifically, this invention relates to self-assembling multi-layer nanocomposite materials of graphene bonded to metal oxides, devices using such materials, methods for forming self-assembling multi-layer nanocomposite materials of graphene bonded to metal oxides and devices using those materials.

BACKGROUND OF THE INVENTION

Graphene is generally described as a one-atom-thick planar sheet of sp2-bonded carbon atoms that are densely packed in a honeycomb crystal lattice. The carbon-carbon bond length in graphene is approximately 0.142 nm. Graphene is the basic structural element of some carbon allotropes including graphite, carbon nanotubes and fullerenes. Graphene exhibits unique properties, such as very high strength and very high conductivity. Those having ordinary skill in the art recognize that many types of materials and devices may be improved if graphene is successfully incorporated into those materials and devices, thereby allowing them to take advantage of graphene's unique properties. Thus, those having ordinary skill in the art recognize the need for new methods of fabricating graphene and composite materials that incorporated graphene.

Graphene has been produced by a variety of techniques. For example, graphene is produced by the chemical reduction of graphene oxide, as shown in Gomez-Navarro, C.; Weitz, R. T.; Bittner, A. M.; Scolari, M.; Mews, A.; Burghard, M.; Kern, K. Electronic Transport Properties of Individual Chemically Reduced Graphene Oxide Sheets. and Nano Lett. 2007, 7, 3499-3503. Si, Y.; Samulski, E. T. Synthesis of Water Soluble Graphene. Nano Lett. 2008, 8, 1679-1682.

While the resultant product shown in the forgoing methods is generally described as graphene, it is clear from the specific capacity of these materials that complete reduction is not achieved, because the resultant materials do not approach the theoretical specific capacity of neat graphene. Accordingly, at least a portion of the graphene is not reduced, and the resultant material contains at least some graphene oxide. As used herein, the term “graphene” should be understood to encompass materials such as these, that contain both graphene and small amounts of graphene oxide.

For example, functionalized graphene sheets (FGSs) prepared through the thermal expansion of graphite oxide as shown in McAllister, M. J.; LiO, J. L.; Adamson, D. H.; Schniepp, H. C.; Abdala, A. A.; Liu, J.; Herrera-Alonso, M.; Milius, D. L.; CarO, R.; Prud'homme, R. K.; Aksay, I. A. Single Sheet Functionalized Graphene by Oxidation and Thermal Expansion of Graphite. Chem. Mater. 2007, 19, 4396-4404 and Schniepp, H. C.; Li, J. L.; McAllister, M. J.; Sai, H.; Herrera-Alonso, M.; Adamson, D. H.; Prud'homme, R. K.; Car, R.; Saville, D. A.; Aksay, I. A. Functionalized Single Graphene Sheets Derived from Splitting Graphite Oxide. J. Phys. Chem. B 2006, 110, 8535-8539 have been shown to have tunable C/O ratios ranging from 10 to 500. The term “graphene” as used herein should be understood to include both pure graphene and graphene with small amounts of graphene oxide, as is the case with these materials.

Further, while graphene is generally described as a one-atom-thick planar sheet densely packed in a honeycomb crystal lattice, these one-atom-thick planar sheets are typically produced as part of an amalgamation of materials, often including materials with defects in the crystal lattice. For example, pentagonal and heptagonal cells constitute defects. If an isolated pentagonal cell is present, then the plane warps into a cone shape. Likewise, an isolated heptagon causes the sheet to become saddle-shaped. When producing graphene by known methods, these and other defects are typically present.

The IUPAC compendium of technology states: “previously, descriptions such as graphite layers, carbon layers, or carbon sheets have been used for the term graphene . . . it is not correct to use for a single layer a term which includes the term graphite, which would imply a three-dimensional structure. The term graphene should be used only when the reactions, structural relations or other properties of individual layers are discussed”. Accordingly, while it should be understood that while the terms “graphene” and “graphene layer” as used in the present invention refers only to materials that contain at least some individual layers of single layer sheets, the terms “graphene” and “graphene layer” as used herein should therefore be understood to also include materials where these single layer sheets are present as a part of materials that may additionally include graphite layers, carbon layers, and carbon sheets.

The unique electrical and mechanical properties of graphene have led to interest in its use in a variety of applications. For example, electrochemical energy storage has received great attention for potential applications in electric vehicles and renewable energy systems from intermittent wind and solar sources. One such energy storage application is Lithium ion (Li-ion) batteries.

Currently, Li-ion batteries are used in a variety of portable electronic devices. As a result of their excellent weight to power ratio, they are also being considered as the leading candidates for hybrid, plug-in hybrid and all electrical vehicles, and possibly for utility applications as well. However, many potential electrode materials (e.g., oxide materials) in Li-ion batteries are limited by slow Li-ion diffusion, poor electron transport in electrodes, and increased resistance at the interface of electrode/electrolyte at high charging-discharging rates.

For Li-ion batteries, SnO₂, Sn and Si are promising high capacity anode materials, but have large volume expansions upon lithiation, causing degradation and rapid fading during charge/discharge cycling. Efforts have been made to prepare composite materials to mix metal oxides and conductive materials such as amorphous carbon, carbon nanotubes and graphene, as discussed in Moriguchi, I.; Hidaka, R.; Yamada, H.; Kudo, T.; Murakami, H.; Nakashima, N. Advanced Materials 2006, 18, 69-73; Zhang, W. M.; Hu, J. S.; Guo, Y. G.; Zheng, S. F.; Zheng, L. S.; Song, W. G.; Wan, L. J. Advanced Materials 2008, 20, 1160; and Huang, H.; Yin, S. C.; Nazar, L. F. Electrochemical and Solid State Letters 2001, 4, A170-A172.

Recently pre-synthesized metal oxide nanoparticles (e.g., TiO₂ and SnO₂) were deposited on graphene surfaces to form nanocomposites as described in Williams, G.; Seger, B.; Kamat, P. V. ACS Nano 2008, 2, 1487-1491; and Paek, S.-M.; Yoo, E.; Honma, I. Nano Letters 2009, 9, 72-75. Other studies, including Niyogi, S.; Bekyarova, E.; Itkis, M. E.; McWilliams, J. L.; Hamon, M. A.; Haddon, R. C. Journal of the American Chemical Society 2006, 128, 7720-7721; Si, Y.; Samulski, E. T. Nano Letters 2008, 8, 1679-1682, Stankovich, S.; Piner, R. D.; Chen, X. Q.; Wu, N. Q.; Nguyen, S. T.; Ruoff, R. S. Journal of Materials Chemistry 2006, 16, 155-158; and Xu, Y. X.; Bai, H.; Lu, G. W.; Li, C.; Shi, G. Q. Journal of the American Chemical Society 2008, 130, 5856, have shown that homogeneous dispersion of the conductive and the active phases remains difficult.

While these results were promising, they fell short of producing materials exhibiting specific capacity approaching the theoretical possibilities. For example, while it has been shown that graphene may be combined with certain metal oxides, the graphene materials in these studies fall far short of the theoretical maximum conductivity of single-sheet graphene. Further, those having ordinary skill in the art recognize that the carbon:oxygen ratio and the specific surface area of graphene provide an excellent proxy to measure the relative abundance of high conductivity single-sheets in a given sample. This is because the C:O ratio is a good measure of the degree of “surface functionalization” which affects conductivity, and the surface area conveys the percentage of single-sheet graphene in the synthesized powder.

Accordingly, those having ordinary skill in the art recognize that improvements to these methods are required to achieve the potential of using graphene nanostructures in these and other applications. Specifically, those skilled in the art recognize the need for new methods that produce nanocomposite materials of graphene and metal oxides that exhibit greater specific capacity and stability than demonstrated in these prior art methods. Further, those of ordinary skill in the art recognize a need for homogeneous dispersion of the conductive and the active phases, and methods for providing such materials.

The present invention fulfills these needs, and provides such improved composite nanostructures of graphene layers and metal oxides that exhibit specific capacities heretofore unknown in the prior art. The present invention further provides improved and novel methods for forming these composite nanostructures, and improved and novel devices that take advantage of the new and unique properties exhibited by these materials. The present invention meets these objectives by making nanostructures of graphene layers and metal oxides where the C:O ratio of the graphene layers in these nanostructures is between 15-500:1, and preferably 20-500:1, and the surface area of the graphene layers in these nanostructures is 400-2630 m2/g, and preferably 600-2630 m2/g, as measured by BET nitrogen adsorption at 77K. While those having ordinary skill in the art have recognized the desirability of having C:O ratios and surface areas this high in the graphene of nanostructures of graphene and metal oxides, the prior art methods have failed to produce them. The present invention further provides homogeneous dispersion of the conductive and the active phases.

SUMMARY OF THE INVENTION

These and other benefits are provided by one aspect of the present invention; a nanocomposite material having at least two layers, each layer consisting of one metal oxide bonded to at least one graphene layer. Typically, the nanocomposite material will have many alternating layers of metal oxides and graphene layers, assembled in a sandwich type construction. Preferably, but not meant to be limiting, the metal oxide used in the nanocomposite material of the present invention is M_(x)O_(y), where M is selected as Ti, Sn, Ni, Mn, Si, V, and combinations thereof.

Also preferably, but not meant to be limiting, in the nanocomposite materials of the present invention at least one layer of the metal oxide is a mesoporous metal oxide. Also preferably, but not meant to be limiting, the nanocomposite material of the present invention is characterized by a specific capacity of greater than about 400 mAh/g.

Preferably, the graphene layers of the nanocomposite materials of the present invention have a thickness between 3 and 20 nm, and more preferably between about 0.5 and 50 nm. Also preferable, but not meant to be limiting, the graphene layers of the nanocomposite materials of the present invention have a carbon to oxygen ratio of between 15 to 1 and 500 to 1 and more preferably between about 20 to 1 and 500 to 1. Also preferably, but not meant to be limiting, the graphene layers of the nanocomposite materials of the present invention have a surface area of between 400 and 2630 m2/g and more preferably between about 600 and 2630 m2/g.

Another aspect of the present invention is a method for forming a nanocomposite material comprising at least two layers, each layer consisting of one metal oxide bonded to at least one graphene layer. This method involves the steps of providing graphene in a suspension; dispersing the graphene with a surfactant; adding a metal oxide precursor; precipitating the metal oxide and allowing the graphene and the metal oxide to organize into self assembled structures.

In this manner, the method of the present invention thereby forms a series of ordered layers, wherein each layer comprises a metal oxide bonded to at least one graphene layer. Those having ordinary skill in the art and the benefit of this disclosure will recognize that the steps of precipitating the metal oxide and allowing the graphene and the metal oxide to organize into self assembled structures may be performed simultaneously, or in either order. Further, those having ordinary skill in the art and the benefit of this disclosure will recognize that while the self assembly process will often result in the metal oxide portions of each successive layer being bound to the graphene portion of an adjacent layer, such is not necessarily the case. For example, and not meant to be limiting, it may be the case that a self assembled structure will form whereby the metal oxide portion of one layer will be bound to the metal oxide portion of a successive layer, or that metal oxide may form into a series of layers. All such self assembled structures should be understood to fall within the invention as described herein, provided that at least two of the layers in that structure comprise a metal oxide bonded to at least one graphene layer.

The suspension of the present invention may be water, or may contain water with other liquids. The method of the present invention may further include the step of precipitating the metal oxide wherein precipitating is maintained for about one to about 24 hours.

Preferably, but not meant to be limiting, the method of the present invention further includes the step of heating the final precipitate from 50 to 500 degrees C. to condense the metal oxide on the graphene surface. Also preferably, but not meant to be limiting, the method of the present invention may further include the step of heating the final precipitate from 50 to 500 degrees C. to remove the surfactant.

The present invention thus includes a nanocomposite material formed by the forgoing method. The nanocomposite material formed by this method is preferably formed into an ordered three-dimensional superstructure having multilength and multiphase building blocks of graphene layers and metal oxide layers, and at least two layers of the nanocomposite material include a metal oxide bonded to graphene. The nanocomposite materials preferably have a thickness between 3 and 20 nm.

While not meant to be limiting, the nanocomposite layers of the present invention find particular utility in energy storage applications. Accordingly, another aspect of the present invention is an energy storage device having a nanocomposite material including at least two layers, each layer having at least one metal oxide bonded to at least one graphene layer. In this application, it is preferred that the nanocomposite material have a specific capacity greater than about 400 mAh/g.

While not meant to be limiting, the nanocomposite layers of the present invention find particular utility as electrochemical devices. In this application, the nanocomposite layers of the present invention have at least one component formed in whole or in part of a nanocomposite material including at least one active metal compound and one graphene layer arranged in a nanoarchitecture. As will be recognized by those having ordinary skill in the art and the benefit of this disclosure, the component may selected as an electrode, an anode, a cathode, a separator, a current collector, an electrolyte, and combinations thereof.

Preferably, but not meant to be limiting, in the embodiment of the present invention where the nanocomposite material is used in the anode of an energy storage device, the anode contains less than 10% carbon-based material by weight, and more preferably less than 5% carbon-based material by weight.

Preferably, but not meant to be limiting, in the embodiment of the present invention where the nanocomposite material is used in the cathode of an energy storage device, the cathode contains less than 5% carbon-based material by weight, and more preferably less than 2.5% carbon-based material by weight.

One example of the present invention that is an electrochemical device and an energy storage device is a lithium ion battery. For example, and not meant to be limiting, one embodiment of the present invention is thus a lithium ion battery having an electrode, wherein the electrode has a nanocomposite material which has at least two layers, each layer including a metal oxide bonded to at least one graphene layer, and wherein said nanocomposite material has a specific capacity of greater than about 400 mAh/g, and wherein each layer includes a metal oxide bonded to graphene, and wherein the layers are provided as an ordered, three dimensional assembly.

As used herein, the term “electrochemical device” includes energy storage devices, energy conversion devices, sensors, and other devices that convert electrical energy to chemical energy, or chemical energy to electrical energy. As used herein, the term “energy storage device” includes batteries and supercapacitors.

BRIEF DESCRIPTION OF THE DRAWINGS

The following detailed description of the embodiments of the invention will be more readily understood when taken in conjunction with the following drawing, wherein:

FIG. 1 is a schematic illustration of the multiphase self-assembly approach of the present invention. 1(A) shows self-assembled hemimicelles on graphite surfaces. 1(B) shows absorption of surfactant hemimicelles on graphene sheets and dispersed macromolecular graphene sheets and surfactant micelles in an aqueous solution. The dispersed graphene sheets can be used as the macromolecular template and the nanophase building block for self-assembly of three-dimensional nanocomposites. 1(C) shows self-assembly of anionic SDS surfactant on graphene surface with oppositely charged metal cation (e.g., Sn²⁺) oxy species into lamella mesophase superstructures toward formation of SnO₂-graphene nanocomposites, where hydrophobic graphene sheets are sandwiched in the hydrophobic domains of the anionic surfactant. 1(D) shows metal oxide-graphene layered superstructures composed of alternating layers of metal oxide nanocrytals and graphene layers after crystallization of metal oxide and removal of the surfactant. 1(E) shows self-assembled hexagonal mesostructure of metal oxide precursor (e.g., silicate) with non-ionic surfactants (e.g., Pluronic P123) with graphene sheets.

FIG. 2(A) to (E) are TEM images of calcined SnO₂-graphene (15 wt % graphene) nanocomposite powder. 2(F) to (H) are TEM images of the NiO-graphene nanocomposite powder. 2(A) is a bright-field cross-sectional TEM image of the SnO₂-graphene nanocomposite powder showing layered structures. The inset is the corresponding SAED pattern. The ring pattern of diffraction shows polycrystalline cassiterite SnO₂. The right symmetrical diffraction spots located at (110) ring corresponds to (001) diffraction of oriented multilayer graphene sheets. 2(B) is a dark-field TEM image obtained from (211) diffraction ring of SnO₂. 2(C) is a dark-field TEM image obtained from the bright (001) diffraction spots of graphene sheets. 2(D) is a high-magnification TEM of SnO₂-graphene nanocomposites in 2(A). The layered structure of SnO₂ is composed of connected nanocrystalline SnO₂ with a 4-5 nm diameter interspaced by graphene layers. 2(E) is a high-resolution TEM image of the layered superstructure of SnO₂-graphene nanocomposites in 2(D). Lattice fringes of 0.33 nm corresponding to (110) plane of SnO₂ and lattice fringes of 0.34 nm corresponding to (001) of multilayer graphene sheets are marked in each layer. 2(F) is a bright-field cross-sectional TEM image of the NiO-graphene nanocomposite (40 wt % graphene) showing nanocrystalline NiO layers (approximately layer thickness of 4 nm) interspaced by graphene layers. The inset is the corresponding SAED pattern showing polycrystalline NiO. 2(G) is a high resolution TEM image of NiO-graphene nanocomposite showing the graphene sheets between NiO layers. Lattice fringes of 0.33 nm corresponding to (001) of multilayer graphene sheets are marked. (H) High resolution TEM image of NiO-graphene nanocomposite showing the lattice fringes of NiO along direction. Lattice fringes of 0.24 nm corresponding to (111) planes in NiO are marked.

FIG. 3( a) is the XRD pattern of the SnO₂-graphene nanocomposite powder (15 wt % graphene). Standard reflection peaks of cassiterite SnO₂ (JCPDS No. 000-0024) are shown as vertical bars. FIG. 3 (b) is the XRD pattern of the NiO-graphene nanocomposite paper showing reflection peaks of (111), (200) and (220) of crystalline NiO, as well as (001) reflection peak of multilayer graphene sheets.

FIG. 4( a) is the cross-sectional TEM image of MnO₂-graphene nanocomposite paper showing layered structures, FIG. 4( b) is the corresponding dark-field TEM image of FIG. 4( a) showing isolated crystalline nanoparticles, indicating amorphous MnO₂ layers coated the graphene surface.

FIG. 5( a) is a photograph of a FGS aqueous dispersion (left) and FGS aqueous dispersion using sodium dodecyl sulfate (SDS) surfactant (right); FIG. 5( b) is a graph showing the UV-Vis absorbance of the SDS-FGS aqueous dispersion. The use of the surfactant sodium 1-dodecanesulfonate in dispersing FGSs in aqueous solution obtains similar results.

FIG. 6(A) is a low angle XRD pattern of the anionic surfactant-SnO₂-graphene precipitates after reaction time of 1 hr (a), 11 hr (b) and 16 hr (c). Lamellar mesophase with (001) d-spacing of 2.3 nm is observed in the mixture. FIG. 6 (B) is a cross-section TEM image of anionic surfactant-SnO₂-graphene precipitates after reaction time of 11 hr. Lamellar mesophase with layer distance of 2.4 nm is marked. FIG. 6 (C) is a TEM image showing worm-like structure of SnO₂ nanocrystals formed through reaction without graphene. FIG. 6 (D) is a cross-sectional TEM image of SiO₂-graphene nanocomposite powder (30 wt % SiO₂). Partially ordered mesoporous silica layers (4-5 mesoporous layer) are observed on the surface of graphene sheets following the contour of wrinked graphene sheets. FIG. 6 (E) is a high-resolution TEM image of the SiO₂-graphene nanocomposite powder in FIG. 6 (D). Graphene sheets are covered with hexagonal mesoporous silica.

FIG. 7 (A) is a side-view SEM image of a self-assembled free-standing SnO₂-graphene nanocomposite (40 wt % graphene) electrode 15-μm thick. Photographs in the inset show a disk-like 3-cm-diameter SnO₂-graphene nanocomposite paper electrode on the left and a bent paper electrode on the right. FIG. 7 (B) is a high-magnification cross-sectional SEM image of the free standing SnO₂-graphene nanocomposite electrode. The electrode is composed of well-packed wavy layers interspaced by the loosely packed layers through almost the entire cross section. FIG. 7 (C) is a schematic illustration of a Li-ion test configuration using a free-standing metal oxide-graphene nanocomposite electrode as an anode. The graphene in the layered superstructures functions as both current collector and conductive additives in the anode. FIG. 7 (D) is a graph showing the charge-discharge profiles of SnO₂-graphene nanocomposite paper electrode (40 wt % graphene) between 0 V and 1.5 V at current densities of 0.008 A/g, 0.02 A/g and 0.08 A/g, respectively. FIG. 7 (E) is a graph showing the specific capacity of SnO₂ as a function of charge-discharge cycles in the SnO₂-graphene nanocomposite paper electrode at current density of 0.01 A/g on top, and the specific capacity of SnO₂ as a function of charge-discharge cycles in the SnO₂-graphene nanocomposite paper at different charge/discharge current density of 0.008 A/g, 0.08 A/g and 0.02 A/g, respectively on the bottom. FIG. 7 (F) is a graph showing the cyclic voltammograms of SiO₂-graphene nanocomposite powder (30 wt % graphene) and FGSs measured in 1M Na₂SO₄ aqueous solution under a scan rate of 2 mV/s with saturated Ag/AgCl as reference electrode.

FIGS. 8 (a,b,c) are cross-sectional TEM images of the SnO₂-graphene nanocomposite paper. FIG. 8 (a) is a low-magnification TEM image, FIG. 8 (b) is a high-magnification TEM image showing the layered superstructure, and FIG. 8 (c) is a high-resolution TEM image showing alternating layers of nanocrystalline SnO₂ and graphene sheets.

FIG. 9 is a graph showing dQ/dV vs. potential plot of lithiated/de-lithiated SnO₂-graphene nancomposites.

FIG. 10 is a graph showing the specific capacity of SnO₂ as a function of charge-discharge cycles in SnO₂-graphene nanocomposite powder (15 wt % graphene) and SnO₂-Super P (40 wt %) at current density of 0.2 A/g.

DETAILED DESCRIPTION OF THE PREFERRED EMBODIMENTS

For the purposes of promoting an understanding of the principles of the invention, reference will now be made to the embodiments illustrated in the drawings and specific language will be used to describe the same. It will nevertheless be understood that no limitations of the inventive scope is thereby intended, as the scope of this invention should be evaluated with reference to the claims appended hereto. Alterations and further modifications in the illustrated devices, and such further applications of the principles of the invention as illustrated herein are contemplated as would normally occur to one skilled in the art to which the invention relates.

A series of experiments were conducted to demonstrate certain embodiments of the present invention. The experimental design is as follows.

Synthesis of SnO₂-Graphene Nanocomposites

In a typical preparation of SnO₂-graphene nanocomposite (e.g., 28 wt % graphene), 71.3 mg of graphene sheets and 12.2 mL of sodium 1-dodecanesulfonate aqueous solution (20 mg/mL, 60° C.) were mixed together. The mixture was diluted by de-ionized H₂O to 30 mL and sonicated for 10-15 min (BRANSON SONIFER S-450A, 400W). 10 mL of 0.1 M SnCl₂ in 3.8 wt % HCl solution was added into as-prepared graphene-surfactant dispersions while stirring. Then, 4.8 mL of 1 M urea was added dropwise under vigorous stirring followed by addition of 4 mL of H₂O₂ solution (1 wt %). Finally, deionized H₂O was added under vigorous stirring until reaching a total volume of 100 mL. For preparation of SnO₂-graphene nanocomposites (40 wt % graphene), 120 mg of graphene sheets and 16.3 mL of sodium 1-dodecanesulfonate aqueous solution were used following the same procedure. The resulting mixture was further stirred in a sealed polypropylene flask at 90° C. for 16 h.

Synthesis of NiO-Graphene Nanocomposites

In a typical preparation of NiO-graphene nanocomposite materials (e.g., 30 wt % graphene), 13 mg of graphene sheets and 1.5 mL of sodium dodecyl sulfate solution (0.5 M) were mixed together. The mixture was diluted by 20 mL of de-ionized H₂O and sonicated for 10-15 min (BRANSON SONIFER S-450A, 400W). Then, 4.06 mL of 0.1 M Ni(NO₃)₂ solution was added dropwise under vigorous stirring followed by addition of 7.29 mL urea solution (0.1 g/L) and 30 mL of de-ionized H₂O. The resulting mixture was further stirred in a sealed polypropylene flask at 90° C. for 16 h. SnO₂-graphene and NiO-graphene nanocomposite precipitates were separated by centrifugation followed by washing with de-ionized H₂O and ethanol. The centrifuge and washing processes were repeated three times. The obtained black powder of SnO₂-graphene and NiO-graphene nanocomposites were then dried in a vacuum oven at 70° C. overnight and subsequently calcined in static air at 400 C for 2 h and in 2.7% H₂/Ar gas at 400 C for 3 h, respectively.

Synthesis of MnO₂-Graphene Nanocomposites

In a typical preparation of MnO₂-graphene nanocomposite materials (e.g., 60 wt % graphene), 5 mg of graphene sheets and 2.5 mL of sodium dodecyl sulfate solution (0.5 M) were mixed together. The mixture was diluted by 20 mL of de-ionized H₂O and sonicated for 10-15 min (BRANSON SONIFER S-450A, 400W). 6 mg of KMnO₄ was dissolved in 10 mL of 0.1 M Na₂SO₄ solution. Then the solution was added dropwise to the surfactant-graphene dispersion under vigorous stirring for 3 h. MnO₂-graphene nanocomposites were obtained by filtration followed by washing with de-ionized H₂O three times. The nanocomposite sample was dried under vacuum overnight followed by heat treatment in atmosphere of 2.7% H₂/Ar gas at 400 C for 3 h.

Fabrication of Metal Oxide-Graphene Nanocomposite Paper Electrodes

Similar to processes of making graphene oxides and graphene papers, vacuum filtration of as synthesized SnO₂-graphene (40 wt % graphene), NiO-graphene (30 wt % graphene) and MnO₂-graphene (60 wt % graphene) nanocomposite solution using Anodisc membrane filters yielded, followed by washing and drying, a free standing metal oxide-graphene nanocomposite paper with thickness ranging from 5 to 20 μm. The metal oxide-graphene nanocomposite papers were then sandwiched between graphite plates and heat treated in an atmosphere of 2.7% H₂/Ar gas at 400 C for 3 h.

Synthesis of Mesoporous SiO₂-Graphene Nanocomposites

0.125 g of poly(ethylene glycol)-b-poly(propylene glycol)-b-poly(ethylene glycol) triblock copolymer (Pluronic P123, EO₂₀PO₇₀EO₂₀, Sigma-Aldrich, USA), 0.5 mL of tetraethyl orthosilicate (TEOS, Sigma-Aldrich), and 0.4 g of 0.1 M HCl were dissolved in 5 mL ethanol. The sol was stirred for 30 min. 0.01 g of graphene sheets was added into the sol followed by vigorous stirring for 15 min. The mixture was dropwise added to a membrane filter under vacuum. The obtained black powders were dried overnight followed by calcination in static air at 400° C. for 2 h. The weight percentage of SiO2 was estimated by TGA measurement.

Characterization

XRD patterns were obtained on a Philips Xpert X-ray diffractometer using Cu K_(α) radiation at λ=1.54 Å. The metal oxide-graphene nanocomposite samples were embedded in resin (LR White Resin, Electron Microscopy Sciences) followed by aging at 60° C. for 20 h. The embedded samples were cross-sectioned by ultramicrotome for TEM studies. The TEM investigation was performed on a JEOL JSM-2010 TEM operated at 200 kV. SEM images were obtained on an FEI Helios Nanolab dual-beam focused ion beam/scanning electron microscope (FIB/SEM) operated at 2 kV.

The Li-ion battery electrochemical evaluations were carried out using half-cell using 2325 coin cells (National Research Council, Canada). Li foil was used as counter and reference electrode. The heat treated SnO₂-graphene nanocomposite paper electrode (40 wt % graphene) was directly used as working electrode without additional electrode preparation. The electrolyte used was 1 M LIPF₆ in ethyl carbonate/dimethyl carbonate (volume ratio 1:1). For preparation of control electrodes using SnO₂-graphene nanocomposite powder (28 wt % graphene) and control SnO₂ powder, a mixture of the active materials, Super P and poly(vinylidene fluoride) (PVDF) binder were dispersed in N-methylpyrrolidone (NMP) solution in a weight ratio of 70:20:10 and 50:40:10, respectively. After stirring overnight the slurry was then coated on the copper foil current collector and dried overnight in air. The coil cells were assembled in an argon-filled glove box. The performance of the SnO₂-graphene nanocomposite paper electrode and the control electrodes were evaluated using Arbin Inst. (College Station, Tex.) at room temperature. The cells were tested between 0.02 V and 1.5 V versus Li metal at various current densities. The specific capacity was calculated based on SnO₂ weight.

The electrochemical capacitor performance of graphene sheets and mesoporous SiO₂ graphene nanocomposites were analyzed with CHI 660c electrochemical workstation (CHI Instruments Inc, Austin, Tex.). All experiments were carried out with a conventional three-electrode configuration in a beaker-type cell. To prepare the working electrode, 5 mg of graphene sheets and mesoporous silica/graphene nanocomposite powder was dispersed in 1 mL of dimethyl formamide or 1 mL of H₂O, respectively. The mixture was sonicated for 5 min. 5 μL of the solution was deposited on glassy carbon electrode and dried in air. 5 μL of a 5% Nafion solution was dropped on the top of the electrode to prevent the loss of the composite material. A platinum wire and an Ag/AgCl electrode were used as the counter and reference electrodes, respectively. The electrolyte was 1M Na₂SO₄ aqueous solution. The specific capacitance was calculated from cyclic voltammograms according to C=I/(m×scan rate), where I represents average current in either positive or negative scan, and m is the mass of single electrode. The real capacitor would operate with a capacitance one-fourth that of the single electrode due to the series connection of two electrodes in real capacitors.

In these experiments, a multiphase self-assembly approach is used to form well-controlled, three-dimensional nanocomposite materials for energy storage from extended nanostructured building blocks. Two-dimensional graphene layers, or sheets, were used as the macromolecular template for the absorption and cooperative assembly of surfactant micelles and metal oxide precursors. As shown in these experiments, the surfactant, metal oxide, and graphene sheets self-assemble into ordered three-dimensional superstructures. The use of these nanocomposite materials for advanced energy storage was then demonstrated. In Li-ion batteries, SnO₂-graphene nanocomposites of the present invention achieved near theoretical specific energy density without significant charge-discharge degradation for Li-ion battery applications. Mesoporous SiO₂-graphene nanocomposites of the present invention showed high specific capacitance for electrical double layer supercapacitors.

In contrast to synthetic approaches, nature has the ability to form nanocomposites with well-controlled architecture from multiscale and multifunctional building blocks. For example, mollusk shells grow distinctive nacreous laminated composites with aragonite nanoplates and organic films between the plates. Coccolith and magnetosom assemble highly organized hierarchical structures from nano- and microcrystalline building blocks. Although in synthetic materials both two-dimensional and three-dimensional molecular templates have been investigated to prepare oriented ceramic thin films, single phase mesostructured inorganics, polymers/surfactants and nanoparticle nanocomposites, self-assembly from multilength and multiphase building blocks has not been successfully demonstrated.

In these experiments, a multiphase self-assembly strategy using both traditional molecular precursors and extended two-dimensional nanosheets as the fundamental building blocks was demonstrated. The formation of complex, self-assembled mesostructures supported on graphite and other substrates has previously been shown. These studies provide some clue for the strategy used to construct three-dimensional, bulk materials. The basic concept is that instead of a graphite substrate, these experiments use two-dimensional nanosheets (graphene) as the macromolecular template for the cooperative absorption and assembly of surfactants and metal oxides on the graphene surface. At the same time, the extended graphene sheets participate in the self-assembly of the surfactant and metal oxide to form ordered three-dimensional superstructures, thus becoming a critical functional component of the nanocomposite materials, as shown in FIG. 1.

Graphene is chosen as a model material because of the high electronic conductivity and good mechanical properties. These experiments used functionalized graphene sheets (FGSs) prepared by thermal expansion process of exfoliated graphene oxide. The surfactant first absorbs to the graphene surfaces as hemimicelles to ensure that the graphene nanosheets are dispersed in the hydrophobic domains of the surfactant micelles. The anionic surfactant simultaneously binds to positively charged metal anions and self-assembles with the graphene to form an ordered lamella mesophase. Subsequently, the metal oxides are crystallized between the graphene, producing a new class of nanocomposites in which alternating layers of graphene sheets and metal oxide nanocrystals are assembled into a layered superstructures.

These experiments focus on the nanocomposites made of metal oxides (e.g., SnO₂, NiO, and MnO₂ etc) that are good candidates for electrochemical energy storage. However, as will be recognized by those having ordinary skill in the art and the benefit of this disclosure, other metal oxides could also be used. One challenge that these experiments overcome is the low conductivity of such materials, which usually requires the addition of a conductive phase to enhance their electron and ion transport. Another challenge that these experiments overcome is the instability of these anode materials upon lithiation (alloying).

For example, when used in Li-ion batteries, SnO₂ is a promising high capacity anode material, but has a large volume expansion upon lithiation, causing degradation and rapid fading during charge/discharge cycles.

FIG. 2 shows the Transmission electron microscopy (TEM) results of the superstructures of alternating nanometer-thick layers of nanocrystalline metal oxides and graphene sheets in SnO₂-graphene and NiO-graphene nanocomposites prepared in the powder form. Cross-sectional TEM image of the calcined SnO₂-graphene nanocomposite prepared clearly shows the regular layers, as shown in FIG. 2A. Each layer is about 3 to 5 nm thick and is rather uniform. A selected area electron diffraction (SAED, inset in FIG. 2A) pattern suggests a typical crystal structure of cassiterite SnO₂ (JCPDS No. 000-0024), which is consistent with the X-ray diffraction (XRD) result shown in FIG. 3. The corresponding dark-field image from the (211) reflection of SnO₂ shown in FIG. 2(b) confirms that the SnO₂ layer is made up of 4-nm nanocrystals. Two symmetrical but diffuse diffraction spots are also observed on top of the (110) diffraction ring of the SnO₂, which are attributed to the (001) reflection of the oriented multilayer graphene sheets. The dark-field image shown in FIG. 2( c) from the (001) reflection of the graphene sheets indeed reveals band structures of the multilayer graphene sheets separated by SnO₂. A high-magnification TEM image shown in FIG. 2( d) reveals that the SnO₂ nanoparticles are connected to one another within the layer but separated from layer to layer by graphene sheets. Lattice fringes of both the (110) plane in 4-nm-diameter nanocrystalline SnO₂ and the (001) plane in multilayer graphene sheets are observed in high-resolution TEM image as shown in FIG. 2( e). Similarly, layered superstructures with alternating layers of metal oxide and graphene sheets are also observed in NiO-graphene, as shown in FIG. 2( f) and MnO₂-graphene nanocomposites as shown in FIG. 4. Lattice fringes of the (001) plane in multilayer graphene sheets and the (111) plane in 5-nm thick nanocrystalline NiO layer are observed in high-resolution TEM images as shown in FIGS. 2( g) and 2(h).

The unique superstructure in the nanocomposites is a direct result of the cooperative self-assembly involving the surfactant, the metal oxide, and nanophase building blocks of graphene sheets. Both experimental and theoretical studies suggested that anionic surfactant molecules absorbed on a graphite surface form tubular, hemicylindrical micelle aggregates. Thus, the anionic surfactant can disperse the FGSs in the hydrophobic domains of the surfactant micelles to form a well-dispersed FGS solution, as shown in FIG. 5. However, when the metal oxide precursor (e.g., SnO₂ precursor) is added to the solution, a black precipitate was obtained with a lamellar mesostructure as revealed by the XRD pattern, as shown in FIG. 6( a). Such a transition from rod-like micelles to lamella structures is caused by the binding of the metal cations with the anionic surfactant head groups which reduces the net charge and the effective head group size, favoring formation of the lamellar mesophase. In addition, the graphene surface might have provided a substrate effect that promotes and stabilizes the lamellar mesophase. Examples of this effect include lamellar mesostructured film on a substrate using SDS as a structural directing agent by evaporation-induced self-assembly or electrochemical deposition.

After formation of the lamellar mesophase, the hydrophobic graphene should still be located in the hydrophobic domain of the lamellar mesophase. Further reaction causes crystallization of SnO₂ between the graphene sheets and leads to degradation of the long-range ordering of the lamellar mesophase as shown in FIG. 6( a), but the overall lamellar mesostructures can be still observed in the TEM image as shown in FIG. 6( b) with an adjacent layer distance of 2.4 nm, consistent with the (001) d-spacing (2.3 nm) observed in the XRD pattern. Finally, calcination results in the decomposition and removal of the surfactants and further growth of SnO₂ nanocrystals forming an interconnected nanocrystalline SnO₂ layer between the graphene sheets. As a comparison, only worm-like nanoporous structures are produced in absence of graphene as shown in FIG. 6( c).

Several layers of graphene sheets are observed between nanocrystalline metal oxide layers. Such multilayers are most likely caused by restacking of graphene due to van der Waals force during reaction, which is a common phenomenon even in the presence of the anionic sulfate surfactant. It is also possible that some of the restacked graphene sheets in the SnO₂-graphene nanocomposites come directly from FGS samples that have not been fully exfoliated. Thus, while the inventors are not certain of the exact mechanism that holds the metal oxide to the graphene layer, it is reasonably suspected to be Van Der Waals forces. However, the invention should not be considered as limited to such arrangements. Accordingly, as used herein the term “bonded” should be understood to include any forces that effectively hold the two materials adjacent to one and another.

An example of nanocomposites made of graphene and hexagonal mesoporous silica is shown in FIGS. 6( d) and 6(e). In this example, a block co-polymer, i.e., Pluronic P123, is used to assist self-assembly of silica on a graphene surface. The nonionic surfactant can adsorb to the graphene surfaces into hemimicelles. However with this surfactant and silica the hexagonal mesophase is more favorable, resulting in a three-dimensional interconnected network of mesoporus silica and graphene sheets.

These experiments then investigated the charge-discharge properties of SnO₂-graphene nanocomposite as the anode for Li-ion batteries. Instead of using the as-prepared powders, the experiments assembled free-standing flexible electrodes in one step without using a binder or current collector. This approach has the potential to directly fabricate energy storage devices through self-assembly. A SEM image of the free-standing SnO₂-graphene nanocomposite electrode, about 15-μm thick, is shown in FIG. 7( a). The SnO₂-graphene nanocomposite electrode in the form of a disk with a diameter of 30 mm is robust and fairly flexible, as shown in the inset of FIG. 7( a). A polished cross-sectional SEM image shown in FIG. 7( b) reveals typical parallel, wavy layer architectures. A cross-sectional TEM image of the SnO₂-graphene electrode shown in FIG. 8 shows similar layered superstructures with alternating layers of nanocrystalline SnO₂ and graphene sheets, as for that in powders, as shown in FIG. 2( a)-FIG. 2( e).

The free standing SnO₂-graphene nanocomposite electrodes were further studied using a half cell design. The coin cell contains a Li metal foil and a separator film of Celgard 2400 saturated with 1M LiPF₆ in ethylene carbonate and dimethyl carbonate (1:1 by volume), as shown in FIG. 7( c). The voltage-capacity profiles of the SnO₂-graphene nanocomposite electrode at different current density are shown in FIG. 7( d). SnO₂ is converted into metallic Sn in the first charge/discharge cycle, as confirmed from differential charge/discharge curves of SnO₂-graphene nanocomposite electrode. In the subsequent charge/discharge cycles, Li ions were reversibly inserted into Sn as Li/Sn alloys (LiSn or Li_(4.4)Sn) as shown in FIG. 9. Pure graphene tested within the same voltage range at current density of 0.004 A/g has a steady capacity of 120 mAh/g. At 40 wt % graphene in the nanocomposites, the capacity from graphene is less than 10% of the total capacity in the SnO₂-graphene electrode. The overall capacity of the electrode is mostly from the SnO₂ active phase.

The specific capacity of the SnO₂ in the nanocomposite paper as a function of cycle number is shown in FIG. 7( e). The discharge capacity drop in 1^(st) cycle is attributed to irreversible conversion of SnO₂ to Sn and Li₂O upon lithiation. The increase in specific capacity during the initial 10 cycles is attributed to improvement in electrolyte wetting of dense SnO₂-graphene nanocomposite electrode and the conversion of SnO₂ to Sn occurring upon initial lithiation. As the electrode is well wetted by the electrolyte, a steady specific capacity of 625 mAh/g is obtained at a current density of 0.02 A/g (as shown in FIG. 7( e), top). Significantly, the SnO₂-graphene nanocomposite electrode shows excellent capacity retention over the charge-discharge cycles in contrast to the rapid degradation of the control SnO₂-Super P electrode, SnO₂-graphene powder electrode as shown in FIG. 10, and typical SnO₂ electrode materials. A steady specific capacity of 760 mAh/g for the nanocomposite paper can be obtained at a current density of 0.008 A/g (shown in FIG. 7( e), bottom), close to the theoretical capacity (780 mAh/g). The specific capacities of 225 mAh/g and 550 mAh/g are obtained at a current density of 0.08 A/g and 0.02 A/g (shown in FIG. 7( e), bottom), respectively. At all the charge rates, the specific capacity in nanocomposite papers is well retained during cycling at different rates. The higher capacity and better stability in the nanocomposite electrodes are attributed to good contact between the nanocrystalline SnO₂ and sandwiched graphene even after conversion and volume change upon lithiation.

High surface area conductive materials with tailored porosity are useful in other energy storage devices such as electrical double layer supercapacitors. These experiments performed a preliminary study on the electrochemical capacitance of the mesoporous SiO₂-graphene nanocomposite powder. FIG. 7( f) shows cyclic voltammograms (CV) using a three-electrode configuration for pure graphene and a mesoporous SiO₂-graphene nanocomposite. Both graphene and the SiO₂-graphene nanocomposite display a capacitive charging current with a rectangular shape across the potential range between −1.0 and 0 V (vs. the saturated Ag/AgCl reference electrode). However, surprisingly the CV response for the nanocomposite with the “inert” silica is significantly enhanced, resulting in a much higher single electrode capacitance of 120 F/g. This value is better than the best result reported in the literature for graphene (about 100 F/g), but the actual specific capacitance for graphene in the nanocomposite is higher (170 F/g) if accounting for the 30 wt % of inert silica. These preliminary studies suggest the improved electrochemical response in the nanocomposites is likely attributed to the open mesoporous network, which prevents aggregation of the graphene sheets on the electrode.

Graphene sheets used in this study were prepared through the thermal expansion of graphite oxide. X-ray photoemission spectroscopy (XPS) of the graphene sheets shows a sharp C1s peak indicating good sp₂ conjugation.

While the invention has been illustrated and described in detail in the drawings and foregoing description, the same is to be considered as illustrative and not restrictive in character. Only certain embodiments have been shown and described, and all changes, equivalents, and modifications that come within the spirit of the invention described herein are desired to be protected. Any experiments, experimental examples, or experimental results provided herein are intended to be illustrative of the present invention and should not be considered limiting or restrictive with regard to the invention scope. Further, any theory, mechanism of operation, proof, or finding stated herein is meant to further enhance understanding of the present invention and is not intended to limit the present invention in any way to such theory, mechanism of operation, proof, or finding.

Thus, the specifics of this description and the attached drawings should not be interpreted to limit the scope of this invention to the specifics thereof. Rather, the scope of this invention should be evaluated with reference to the claims appended hereto. In reading the claims it is intended that when words such as “a”, “an”, “at least one”, and “at least a portion” are used there is no intention to limit the claims to only one item unless specifically stated to the contrary in the claims. Further, when the language “at least a portion” and/or “a portion” is used, the claims may include a portion and/or the entire items unless specifically stated to the contrary. Likewise, where the term “input” or “output” is used in connection with an electric device or fluid processing unit, it should be understood to comprehend singular or plural and one or more signal channels or fluid lines as appropriate in the context. Finally, all publications, patents, and patent applications cited in this specification are herein incorporated by reference to the extent not inconsistent with the present disclosure as if each were specifically and individually indicated to be incorporated by reference and set forth in its entirety herein. 

1. A method comprising: forming an ordered nanocomposite material by providing graphene layers having a first surface and a second surface; dispersing the graphene layers with a surfactant in a suspension; adding a metal oxide precursor; precipitating metal oxide in a manner to form a self-assembled nanocomposite material having a plurality of ordered layers, at least two of the ordered layers consisting essentially of a metal oxide layer directly bonded to a first surface of a graphene layer, wherein the at least two ordered layers are bonded to one another such that the metal oxide layers and graphene layers are alternatingly positioned in the ordered layers.
 2. The method of claim 1 wherein the graphene layers consist essentially of functionalized graphene sheets.
 3. The method of claim 1 wherein the graphene layers consist essentially of 1 to 127 graphene sheets.
 4. The method of claim 1, wherein the step of precipitating is maintained for about one to about 24 hours.
 5. The method of claim 1 wherein the graphene and surfactant suspension further comprises water.
 6. The method of claim 1 further comprising the step of heating the precipitate from 50 to 500° C. to condense the metal oxide on the graphene surface.
 7. The method of claim 6 further comprising heating the precipitate from 50 to 500° C. to remove the surfactant.
 8. The method of claim 1 further comprising the step of calcining the precipitate.
 9. The method of claim 1 wherein the metal oxide is M_(x)O_(y), and where M is Ti, Sn, Ni, Mn, V, Si, or Co, or is a combination thereof.
 10. The method of claim 1 wherein the metal oxide is titania.
 11. The method of claim 1 wherein the metal oxide is tin oxide.
 12. The method of claim 1 wherein the metal oxide is mesoporous.
 13. The method of claim 1 wherein the graphene layers have a carbon to oxygen ratio of 10-500:1.
 14. The method of claim 1 wherein the nanocomposite material formed is an ordered three-dimensional superstructure having multilength and multiphase building blocks of the graphene layers and the metal oxide layers, and wherein the graphene layers in the superstructure have thicknesses of less than 20 nm.
 15. The method of claim 1 wherein the surfactant is sodium dodecyl sulfate.
 16. A method comprising: forming an ordered nanocomposite material by dispersing graphene layers with a surfactant wherein the graphene layers consist essentially of 1 to 127 graphene sheets; adding a metal oxide precursor to the dispersed graphene layers to form a mixture; forming a self-assembled nanocomposite material having a plurality of ordered layers by heating the mixture to crystallize mesoporous metal oxide onto surfaces of the graphene layers in the mixture, wherein at least two of the ordered layers consist of a mesoporous metal oxide layer bonded directly to a first surface of a graphene layer, wherein the at least two ordered layers are bonded to one another such that the mesoporous metal oxide layers and graphene layers are alternatingly positioned in the ordered nanocomposite material.
 17. The method of claim 16 wherein each of the graphene layers consists of 1 to 127 graphene sheets. 